C6 Rates of Reaciton

Trim End | 03:44

Question 1 | 00:00

Question 2 | 00:44

Question 3 | 01:25

Question 4 | 01:34

Question 5 | 01:59

Question 6 | 02:26

Question 7 | 03:24

00:00/00:00

Question 1

00:00

Question 2

00:44

Question 3

01:25

Question 4

01:34

Question 5

01:59

Question 6

02:26

Question 7

03:24

Trim End | 05:03

Questions 8 & 9 | 00:17

Question 10 | 01:19

Question 11 | 01:51

Question 12 | 02:28

Question 13 | 03:09

Question 14 | 03:24

Question 15 | 04:07

Question 16 | 05:00

00:00/00:00

Questions 8 & 9

00:17

Question 10

01:19

Question 11

01:51

Question 12

02:28

Question 13

03:09

Question 14

03:24

Question 15

04:07

Question 16

05:00

1

What is the volume of gas in the syringe?

Volume = _______ cm3

WS2.3

1

Which apparatus would measure 50cm3 of hydrochloric acid with the greatest accuracy

WS2.4

1

The student measured the volume of gas produced every 20 seconds for 2 minutes.

The volume of gas was zero at the start of the experiment.

The measured volumes of gas were: 26 cm3 38 cm3 47 cm3 55 cm3 59 cm3 60 cm3

Complete the table to show these results.

Tick one box to select the correct unit for each variable.

MS2c

2

Describe the trends shown in the student’s results.

4.6.1.1

WS3.5

1

4.6.1.1

MS4a

1

4.6.1.1

MS4a

1

4.6.1.1

MS3c

1

Match the method to the unit of rate of reaction

Draggable item		Corresponding Item
Marble chips in hydrochloric acid are placed in a conical flask, with a bung attached to a gas syringe at the opening.		g/s
A conical flask containing sodium thiosulfate and dilute hydrochloric acid is placed on a piece of paper with a cross on it.		cm3/s
Marble chips and hydrochloric acid are placed in a conical flask on a top-pan balance.		s

4.6.1.1

2

Describe the trends shown in the student’s results.

4.6.1.1

WS3.5

1

The symbol equation for the decomposition of hydrogen peroxide (H2O2) is: 

2 H2O2 → 2 H2O + O2 

Complete the word equation for the decomposition of hydrogen peroxide. 

hydrogen peroxide → _______ + _______

4.6.1.1

1

Measuring the gas produced, the mass lost, or the light transmitted are all ways of measuring the rate of reaction.

4.6.1.1

6

Describe to Jun a method he could use to measure rate of reaction, and an advantage of using this method.

4.6.1.1

1

Increasing the pressure of gases in a reaction will increase the rate of reaction.

4.6.1.2

1

Increasing the temperature of reactants increases the number of particles in the reaction.

4.6.1.2

1

There are five main factors that affect the rate of reaction.

4.6.1.2

WS1.3

1

For every 10°C temperature increase, the rate of reaction triples.

4.6.1.2

1

Collision theory states that particles must collide with enough energy in order to react.

4.6.1.3

1

The minimum amount of energy required for a successful collision is called the starter energy.

4.6.1.3

1

Different catalysts are needed for different reactions.

4.6.1.4

1

During a reaction, a catalyst gets used up and has to be replaced each time.

4.6.1.4

1

Catalysts are usually cheap transition metals.

4.6.1.4

C6 Rates of Reaciton

Which apparatus would measure 50cm3 of hydrochloric acid with the greatest accuracy

Describe the trends shown in the student’s results.

Match the method to the unit of rate of reaction

Describe the trends shown in the student’s results.

Measuring the gas produced, the mass lost, or the light transmitted are all ways of measuring the rate of reaction.

Describe to Jun a method he could use to measure rate of reaction, and an advantage of using this method.

Increasing the pressure of gases in a reaction will increase the rate of reaction.

Increasing the temperature of reactants increases the number of particles in the reaction.

There are five main factors that affect the rate of reaction.

For every 10°C temperature increase, the rate of reaction triples.

Collision theory states that particles must collide with enough energy in order to react.

The minimum amount of energy required for a successful collision is called the starter energy.

Different catalysts are needed for different reactions.

During a reaction, a catalyst gets used up and has to be replaced each time.

Catalysts are usually cheap transition metals.

Which apparatus would measure 50cm3 of hydrochloric acid with the greatest accuracy

Describe the trends shown in the student’s results.

Match the method to the unit of rate of reaction

Describe the trends shown in the student’s results.

Measuring the gas produced, the mass lost, or the light transmitted are all ways of measuring the rate of reaction.

Describe to Jun a method he could use to measure rate of reaction, and an advantage of using this method.

Increasing the pressure of gases in a reaction will increase the rate of reaction.

Increasing the temperature of reactants increases the number of particles in the reaction.

There are five main factors that affect the rate of reaction.

For every 10°C temperature increase, the rate of reaction triples.

Collision theory states that particles must collide with enough energy in order to react.

The minimum amount of energy required for a successful collision is called the starter energy.

Different catalysts are needed for different reactions.

During a reaction, a catalyst gets used up and has to be replaced each time.

Catalysts are usually cheap transition metals.

What is rate?

What reaction is most suitable to measure rate?

Select the correct equations for calculating rate of reaction

What are suitable units of rate?

What is always the correct unit of time?

We produce 10g in 2 minutes. What is the average rate of reaction?

At the beginning of a chemical reaction, the rate is....

What two pieces of measuring equipment is he going to use to capture gas is this experiment?

What pieces of equipment is best for measuring the volume of a liquid, like acid?

Which piece of equipment is he using to capture gas in the first method?

How often do you need to measure the gas produced?

The first time he did this, he used 2 mol/dm3. The second time time he is using 1 mol/dm3. Do you think it will be faster or slower?

What piece of equipment captures the gas in this second experiment?

What piece of equipment measures time for all his experiments?

What do both experiments level off at the same point?

List the 3 sources of error from the video